Why can't molecules of a covalent compound conduct electricity?

• A. Because covalent compounds do not have free ions or electrons to carry an electric current.
• B. Because covalent compounds are always solids at room temperature.
• C. Because covalent compounds are always polar.
• D. Because covalent compounds have strong metallic bonds.

Answer: (A)

Verified step by step guidance

1. Understand that electrical conductivity in substances depends on the presence of charged particles, such as free ions or free electrons, that can move and carry charge through the material.
2. Recall that covalent compounds are formed by atoms sharing electrons to form molecules, and these molecules are electrically neutral overall, meaning they do not have free ions.
3. Recognize that in covalent compounds, electrons are localized in bonds between atoms and are not free to move throughout the substance, unlike in ionic compounds or metals.
4. Note that because there are no free charged particles (ions or electrons) in covalent compounds, they cannot conduct electricity in solid or liquid form.
5. Conclude that the inability of covalent compounds to conduct electricity is due to the absence of free ions or electrons, not because of their physical state, polarity, or bonding type.